The pH of a 0.045 M Ca(OH)2 solution is: +1.3467 O +12.954 O +12.653 O -1.3467

Q: If you have 0.1 x 6x 10^23 hydrogen ions in 1L of solution, what is the pH? O A. 7 В.3 O C. 5 O D.…

A: The correct answer is given below

Q: What is the pH of a 0.65 M solution of pyridine, C5H5N?

A: Given,  The concentration of C5H5N is 0.65M The kb value of C5H5N is 1.7×10-9 To solve: pH of 0.65M…

Q: The pH of an aqueous solution of 0.413 M triethylamine (a weak base with the formula (C2H3)N) is

A: The value of base dissociation constant ,Kb, of ethylamine is 5.6 . 10-4  ethylamine is a weak base…

Q: The pH of a 0.064-M solution of hypobromous acid (HOBR but usually written HBrO) is 4.97. Calculate…

A:

Q: em101 The pH of a 0.0049 M solution of Ca(OH), is

A: Given that: molarity of Ca(OH)2 = 0.0049 M To find: pH of 0.0049 M Ca(OH)2 solution?

Q: The pH of a 0.063-M solution of hypobromous acid (HOBR but usually written HBRO) is 4.93. Calculate…

A: We will use weak acid concept.

Q: Find the pH of a solution whose [OH] is 2.8 x 10 5 M. O 2.8 O 9.4 O 4.6 O 13

A: Using relation between pH and pOH we can find pH.  Given [OH-] = 2.8 * 10-5M

Q: What is the pH of a 3.21 ×10 -2 M solution of KOH?   1.49 9.97 12.5 6.97

A: Given, Concentration of the KOH solution = 3.21 ×10 -2 M  pH of a 3.21 ×10 -2 M solution of KOH = ?…

Q: The pH of a 0.10 M solution of formic acid (HCOOH) is 2.39. What is the Ka of the acid?

A: pH is the universal indicator , that not only help in detecting the acidic/ basic character but also…

Q: The pH of a 0.55 M aqueous solution of hypobromous acid, HB1O, at 25.0 °C is 4.48. What is the…

A: The percentage of ionization of HBrO can be calculated as follows

Q: is the pH of orange juice when the hydrogen ion concentration is 0.0005 M. O 3.3 O 2.3 O 4.3 O 5.3

A:

Q: what is the pH of a 0.140 M solution of NH4Cl? ka for ammonium is 5.68x10^-5

A: A salt that contains either weak acid ions or weak base ions does not exact 7 pH values. Its pH…

Q: What is the pH of a 0.250 M HOCI solution? K, of HOCI at 25°C is 3.5 x 10-8. O 7.46 O 4.03 O 3.57 O…

A: ​Given - - - >   Ka = 3.5*10-8   pH = 0.25

Q: The concentration of H* (or H3O*) from part A should be 1.02x×10-2 mol L-1. What is the pH of the…

A:

Q: Nitrous acid (HNO2), is a monoprotic acid with an ionization constant of 3.98 x 104. Calculate the…

A: Ionisation constant (i.e. ka) = 3.98 × 10-4  Concentration of HNO2 = 0.25 M  pH of the solution = ?

Q: A 0.125 M weak acid (HA) solution has a pH of 2.25. Find the acid ionization constant, Ka-

A: Given that : Initial concentration of weak acid = 0.125 M pH = 2.25 The pH can be given by : pH =…

Q: Calculate the pH of a 0.188 M NH3 solution. The Kb of NH3 is 1.76 x 10-5 O 5.480 O 12.656 O 11.260…

A: NH3 dissociates in water as,                                     NH3 +H2O -----> NH4+ + OH-…

Q: The poison strychnine is a weakly basic compound with Kb = 1.8 x 10 What is the pH of a 0.058 M…

A: Given that, 0.058 M solution of a weak base, i.e. C = 0.058 M. The Kb is 1.8×10-6. We have to…

Q: What is the pH of a 0.0138 M solution of pyridine (C5H5N), a weak base?

A:

Q: The pH of a 0.02 M NgOH solution at 25 °C is: O 12.8 O 13.7 O 1 1.5 O 12.3 O 13.1

A:

Q: A diprotic acid, H:A, has Ka1 = 3.4 × 104 and Ka2 = 6.7 × 10-°. What is the pH of a 0.17 M solution…

A:

Q: the concentration of H3O+ of seawater is 3.16 x 10-9. what is the pH of seawater?

A: Ph depends on concentration of H+ ions...

Q: The pH of an acetic acid (Ka = 1.75 x 10−5) solution is 3.14.  What is the concentration of acetic…

A: Given :-  pH of acetic acid solution = 3.14  Ka for acetic acid = 1.75 × 10-5  To be calculated :-…

Q: Calculate the percent ionization of a 0.125-M solution of nitrous acid (a weak acid), with a pH of…

A: pH of a solution is equal to negative logarithm of the concentration of the hydrogen ion. Write the…

Q: A beaker holds a mixture of 0.40 M HIO3 and 1.0 M HCOOH. Ka(HIO3) = 1.6 x 10-1 Ка(нсоон) = 1.77 ×…

A: Given: Ka (HIO3) = 1.6 × 10-1 Ka (HCOOH) = 1.77 × 10-4 We have to calculate the pH of a mixture of…

Q: The pH of a 0.05 M NaOH solution at 25 °C is: O 13.8 O 13.1 O 1.5 • 12.7 O 10.3

A:

Q: Given that the Ka of a monoprotic acid HA is 3.20 x 10, and the acid HA concentration is 0.751 M,…

A:

Q: Calculate the pH of a solution in which the molar concentration of H+ is 1.6 x 10-9. a. 1.60 b.…

A: Given information,     Molar concentration of H+ is 1.6 x 10-9.

Q: Question is attached

A: Given information: Concentration of dimethylamine = 0.393 M

Q: What is the pH of the following solutions? [H+] = 1.5 × 10-3 M ▪ [H+] = 8.7 × 10-12 M %3D [OH-] =…

A: The solutions are given below -

Q: Calculate the pH of a solution that is 0.15 M NH3 and 0.35 M NHẠNO3. (Kb = 1.8 x 105) NH3 (aq) H20…

A: Hey, since you have asked multiple question, we will solve the first question for you. If you want…

Q: The pH of a 0.05 M NaOH solution at 25 °C is: O 10.3 O 12.7 O 11.5 O 13.1 O13.8

A: pH of solution is calculated using relation pH + pOH = 14

Q: If the [OH] of and acid is 2.57 x 10-8, what is the pH? o 13.2 o 12.49 ○ 6.41 o 2.91

A:

Q: 1.21 х 103 М HNO3

A: Calculate the pH of each of the following solutions of strong acids.

Q: The PH in a 0.005 M solution of Ba(OH), is: O 14 O 13 O 5 O 12

A:

Q: NH3 is a weak base (?b=1.8×10−5Kb=1.8×10−5) and so the salt NH4Cl acts as a weak acid. What is the…

A:

Q: The pOH of an aqueous solution of 0.371 M dimethylamine (a weak base with the formula (CH2),NH) is

A: Given: Concentration of dimethylamine = 0.371 M Kb of = 5.9×10-4

Q: What is the pH of ammonium bromide solution with a concentration of 0.563 M. The base ionization…

A:

Q: The pH of a 1.00 M solution of urea, a weak organic base, is 7.050. Calculate the Ka of protonated…

A: [CH4N2O] = 1.00 M pH = 7.050 Calculating the [H3O+] from the given pH value, pH = -log[H3O+] [H3O+]…

Q: Why is the pH of water at 25oC equal to 7.00?

A:

Q: The hydronium ion concentration of an aqueous solution of 0.558 M isoquinoline (a weak base with the…

A:

Q: The pH of an acidic aqueous solution with a pOH of 9.25

A: Given data is as follows: The pOH of the aqueous solution = 9.25 The pH of the aqueous solution = ?…

Q: Exactly 250 ml solution was made by dissolving 0.01 g of NaOH in water. What is the PH for the…

A:

Q: Question attached

A: pH of solution is measure the acidity or basicity of solution and it calculated by the following…

Q: The pH of an aqueous solution of 0.390 M methylamine (a weak base with the formula CH;NH2) is

A: 12.09

Q: What is the pH of an aqueous solution at 25.0 °C in which [OH ]is 0.0045 M? O 2.35 O -11.65 O 11.65…

A: Answer: option c) 11.65 is the pH of the solution.

Q: If the pH of a 0.0850 M solution of HBrO2 is 2.29, then what is the value for the acidity constant,…

A: pH = -log[H+] Relation between [H+], Ka and C of a weak acid solution: [H+] = (Ka x C)1/2

Q: The pH of a solution containing a hydrogen ion concentration of 1 x 10-5 is:  A. 3 and its pOH is 6…

A:

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.